Question

The valence bond structure of carbon monoxide is best described as: $C \equiv O$ with a dative bond from oxygen atom to the less electronegative carbon atom.
If true enter 1 else 0.

Answer 1

To solve such questions ,we should have the knowledge of different kinds of chemical bonds existing between the molecules. Here, Carbon monoxide is the simplest oxocarbon with one carbon and one oxygen atom. It has empty sp hybrid orbitals. It is tasteless, odourless and colourless gas flammable in nature.

Complete answer:
In carbon monoxide, one carbon atom and one oxygen atom is bonded by a triple bond. That means the carbon monoxide atom consists of one sigma and two pi bonds. The valence bond structure of a molecule explains the way in which the atomic orbitals of the atoms combine to lead the formation of new chemical bonds upon the formation of the molecule.

In case of carbon monoxide, the atomic number of carbon is 6. This leads to the electronic configuration of carbon atoms as $1{s^2}2{s^2}2{p^2}$. Due to this configuration, there is a formation of two $sp$ hybrid orbitals. One of the $sp$-hybrid orbits is directed towards the oxygen and the other opposite to it. As a result, $sp$hybridised singly occupied forms sigma and pi bonds with p-orbitals.

Due to which the ${p_y}$ is empty orbital and ${p_y}$ of the oxygen atom is doubly occupied. Then there is again a formation of pi bond which is formed by the lone pair of oxygen atom and ${p_y}$ atomic orbital of carbon atom.

Hence, 1 i.e. there exists a dative bond between carbon and oxygen.

Note: According to the Molecular Orbital Theory ,three types of orbitals exist-bonding ,non-bonding and antibonding orbitals. The antibonding orbitals of carbon monoxide are empty in nature and this empty orbital accepts electrons from metal during the bonding of metal with carbon monoxide. This is also known as the lowest occupied molecular orbital.